Question

What is the molarity of a solution that contains 2.35 g of nh3 in 0.0500 l of solution?

Answer 1

Answer:

M = 2.76 M

Explanation:

To calculate the molarity of any solution, we need to use the following expression:

M = n/V  (1)

Where:

M: Molarity of solution (mol/L or M)

n: moles of NH3 (moles)

V: volume of solution (In Liters)

But we do not have the moles of NH3, so it needs to be calculated. We have the mass and we can use the following expression to calculate the moles:

n = m/MM (2)

Where:

m: mass of NH3 (g)

MM: molar mass of NH3 (g/mol)

The reported molar mass of NH3 is 17.031 g/mol, so, using the mass of NH3 and this MM, we can calculate the moles:

n = 2.35 / 17.031 = 0.138 moles

With these moles, we can calculate the molarity:

M = 0.138 / 0.05

M = 2.76 mol/L

And this is the concentration or molarity of the NH3 solution.

Answer 2

The molarity of a solution that contains 2.35 g of NH₃ in 0.0500 l of the solution is 2.76 M.

What is molarity?

Molarity is the measure of the concentration of any solute per unit volume of the solution.

$\rm M = \dfrac{n}{V}$

Mass is 2.35g

The volume of  NH₃ is 0.0500 l                

First, calculate the number of moles

The molar mass of  NH₃ is 17.031g/ml

$\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}$

$\rm Number\;of \;moles= \dfrac{2.35}{17.031 g/mol} = 0.138\; moles$

Now, we have moles and volume, so we can calculate the molarity

Putting the values in the first equation

$\rm M = \dfrac{0.138}{0.0500\;l} = 2.76 mol/L$

Thus, the molarity of a solution that contains 2.35 g of NH₃ in 0.0500 l of the solution is 2.76 M.

Learn more about molarity

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